1、NOMENCLATURE,OF IONIC,COMPOUNDS,By John Weide with modifications by Ken Costello,IONIC COMPOUNDS,Compounds are two or more elements that are held together by opposite charge attraction.,Oxygen-8,Magnesium-12,8 (+) 10 (-) -2 Charge,12 (+) 10 (-) +2 Charge,Metal,Non-metal,Metals combine with non-metal
2、s Metals loose electrons to non-metals They then attract because their charges will be opposite.,Metals,Negative Ions (single atoms),-3,-2,-1,Most of the negative ions have a set negative charge,+1,+2,+3,+1,+2,-3,-2,-1,For example the oxy-salts of chlorine, bromine and iodine have many trends in com
3、mon. Look for them below,The next table contains the polyatomic ions that need to be committed to memory. Remember to learn the name, formula and oxidation number,POLYATOMIC IONS (charged building blocks) Polyatomic ions are mostly made of two non-metals.,Ions with -1 charge perbromate BrO4-1 bromat
4、e BrO3-1 bromite BrO2-1 hypobromite BrO-1 perchlorate ClO4-1 chlorate ClO3-1 chlorite ClO2-1 hypochlorite ClO-1 periodate IO4-1 iodate IO3-1 iodite IO2-1 hypoiodite IO-1,nitrate NO3-1 nitrite NO2-1hydroxide OH-1 cyanide CN-1acetate C2H3O2-1 Permanganate MnO4-1 bicarbonate HCO3-1Ions with a -2 Charge
5、 carbonate CO3-2 sulfate SO4-2,sulfite SO3-2 chromate CrO4-2 dichromate Cr2O7-2 oxalate C2O4-2Ions with a -3 Charge phosphate PO4-3 phosphite PO3-3 arsenate AsO4-3Ions with +1 charge ammonium ion NH4+1,Ions with -1 charge perbromate BrO4-1 bromate BrO3-1 bromite BrO2-1 hypobromite BrO-1 perchlorate
6、ClO4-1 chlorate ClO3-1 chlorite ClO2-1 hypochlorite ClO-1 periodate IO4-1 iodate IO3-1 iodite IO2-1 hypoiodite IO-1,-1,These polyatomic ions match the charge of the single element,-2,These polyatomic ions match the charge of the single element,Ions with a -2 Chargesulfate SO4-2 sulfite SO3-2Ions wit
7、h a -3 Charge phosphate PO4-3 phosphite PO3-3,-3,It is also important to memorize the oxidation of the ions that have fixed oxidation numbers (positive or negative). In particular, those from groups 1A, 2A, 3A, 4A, 5A, 6A, 7A, 8A and the elements: Zn, Cd and Ag. Use the following periodic chart to d
8、etermine their oxidation numbers. Just click on the element symbol,N,Elements with Fixed Oxidation Numbers,La,Hf,Ta,Re,Os,Ce,Ba,Tl,Pb,Bi,Po,At,Rn,Ir,Pt,Au,Hg,Y,Zr,Nb,Mo,Tc,Ru,Rb,Sr,In,Sn,Sb,Te,I,Xe,Rh,Pd,Ag,Cd,Sc,Ti,V,Cr,Mn,Fe,K,Ca,Ga,Ge,As,Se,Br,Kr,Co,Ni,Cu,Zn,Al,Si,P,S,Cl,Ar,Na,Mg,B,C,O,F,Ne,Li,Be
9、,H,H,He,Ac,Rf,Db,Sg,Rh,Hs,Fr,Ra,Mt,+1,+2,+3,1A,2A,8A,0,-4,-3,-2,-1,7A,6A,5A,4A,3A,W,Click on element to see its oxidation number(s),Next Slide,Naming Ionic Compounds,The positive ion (usually a metal) is named first while the negative ion (a non-metal or a polyatomic ion) is named last.The charge on
10、 the negative ion is used to determine the charge on the positive ion. In-order for the total oxidation state to be zero, the total positive charge must equal the total negative charge. A simple algebraic equation can be used to determine the charge on a single metal ion. This charge is expressed as
11、 a “Roman Numeral” in parenthesis that immediately follows the name of the metal.,CuSO4 Cu?SO4-2 x +(-2)=0 X = 2,Copper (II) Sulfate,Naming Ionic Compounds,The positive ion (usually a metal) is named first while the negative ion (a non-metal or a polyatomic ion) is named last.The charge on the negat
12、ive ion is used to determine the charge on the positive ion. In-order for the total oxidation state to be zero, the total positive charge must equal the total negative charge. A simple algebraic equation can be used to determine the charge on a single metal ion. This charge is expressed as a “Roman
13、Numeral” in parenthesis that immediately follows the name of the metal.,Cu2SO4 Cu2+xSO4-2 2x +(-2)=0 x = 1,Copper (I) Sulfate,Naming Ionic Compounds,If the positive ion is one that has a fixed oxidation number then no Roman Numeral is used. Everyone should know the charge of fixed ions. These includ
14、e metals in group 1A, 2A and the specific metals: Al, Zn, Cd & Ag (zinc, cadmium and silver).,CaSO4,Calcium Sulfate,No Roman Numeral,If the ionic compound is binary it will end in “-ide”. However, not all compounds that end in “-ide” are binary. For example sodium hydroxide has the formulaNaOH (thre
15、e different kinds of atoms).If the negative ion is a polyatomic ion the compound is no longer binary. The ending will be that carried by the polyatomic ion. These endings are either “-ate” or “-ite.”Hydrated compounds are named using a combination of both the stock system and prefixes. A prefix is u
16、sed to denote the number of water molecules attached to the ionic formula. “hydrate” is used as the name indicating that water is attached. For example, copper(II) sulfate pentahydrate has the formula CuSO4.5H2O,Examples #1- Formulas to Names,CuSO3,copper,Im a polyatomic ion,1. Write the names of th
17、e ions,Final Name,sulfite,(II),x,X + (- 2) = 0,X = +2,Cu,SO3,= 0,You must know the charge on the sulfite ion is -2,The sum of the positive and negative charges must equal zero,2. Determine the charge of the positive ion,-2,+2 +2,Next,+2,Examples #2- Formulas to Names,KMnO4,potassium,Im a polyatomic
18、ion,1. Write the names of the ions,Final Name,permanganate,If the positive ion has a fixed charge, you are finished.,Examples #3- Formulas to Names,NH4NO3,ammonium,Im a polyatomic ion,2. Determine the charge of the positive ion,1. Write the names of the ions,Final Name,nitrate,If the positive ion ha
19、s a fixed charge, you are finished.,Examples #4- Formulas to Names,SnF2,tin,2. Determine the charge of the positive ion,1. Write the names of the ions,Final Name,fluoride,(II),Snx (F-1)2 = 0,X + 2(-1) = 0,X = +2,Examples #5- Formulas to Names,Ba(ClO4)2,barium,Im a polyatomic ion,2. Determine the cha
20、rge of the positive ion,1. Write the names of the ions,Final Name,perchlorate,If the positive ion has a fixed charge, you are finished.,Examples #6- Formulas to Names,Cu2S,copper,Im not a polyatomic ion,2. Determine the charge of the positive ion,1. Write the names of the ions,Final Name,sulfide,(I)
21、,2Cux (S)-2 = 0,2X + (-2) = 0,X = +1,Examples #6- Formulas to Names,Cu2S,copper,1. Write the names of the ions,Final Name,sulfide,(I),x,2X + (- 2) = 0,2X = +2,(Cu )2,S,You must know the charge on the sulfide ion is -2,The sum of the positive and negative charges must equal zero,2. Determine the char
22、ge of the positive ion,-2,+2 +2,Next,+1,X = +1,Examples #7- Formulas to Names,Na2Cr2O7,sodium,Im a polyatomic ion,2. Determine the charge of the positive ion,1. Write the names of the ions,Final Name,dichromate,(I),2(Nax)(Cr2O7)-2 = 0,2X + (-2) = 0,X = +1,If the positive ion has a fixed charge, it i
23、s not shown,Examples #10- Formulas to Names,LiCN,lithium,Im a polyatomic ion,2. Determine the charge of the positive ion,1. Write the names of the ions,Final Name,cyanide,If the positive ion has a fixed charge, you are finished.,Writing Ionic Formulas,It is easier to write the formula of an ionic co
24、mpound from its name than the reverse. The oxidation number of the negative ion must be memorized in all cases. Refer to the table of polyatomic ions.,aluminum chloride,What is the Lowest Common Multiple “LCM” of 3 and 1. Do not worry about the sign(+/-),Example #1-Names to Formulas,Al,Cl,3,2. Deter
25、mine number of ions,1. Write symbols of elements,Final Formula,(Al )x(Cl-1)y= 0,1,If there is only one atom the “1” is not shown,+3,If there is no Roman Numeral, you need to know the fixed oxidation number of the positive ion.,Next,Example #1-Names to Formulas,aluminum chloride,Al,Cl,3,2. Determine
26、number of ions,1. Write symbols of elements,Final Formula,x(+3) + y(-1) = 0,1,For aluminum, a 1 is multiplied times the +3 to give a +3 charge,If there is only one atom the “1” is not shown,If there is no Roman Numeral, you must know the oxidation number of the positive ion.,+3,If there is no Roman
27、Numeral, you must know the oxidation number of the positive ion.,What is the Lowest Common Multiple “LCM” of 3 and 1. Do not worry about the sign(+/-),(Al )x(Cl-1)y,What is the Lowest Common Multiple “LCM” of 3 and 1. Do not worry about the sign(+/-),For chloride, a 3 is multiplied times the -1 to g
28、ive a -3 charge,1(+3) + 3(-1) = 0,Remember all compoundsare neutral, thus the total positive charge must equal the total negative charge,Next,This formula says that the +3 charge of one Al atom will cancel the-3 charge from 3 Cl atoms,Example #2-Names to Formulas,cobalt(II) bromate,Co,BrO3,2. Determ
29、ine number of ions,1. Write symbols of elements,Final Formula,(Co+2)x(BrO3-1)y= 0,2X = 1y,X(+2) + y(-1) = 0,1,Choose the lowest set of integers that satisfies the equation,(BrO3)2,If there is only one atom the “1” is not shown,Next,Example #3-Names to Formulas,nickel(III) acetate,Ni,C2H3O2,2. Determ
30、ine number of ions,1. Write symbols of elements,Final Formula,(Ni+3)x(C2H3O2-1)y= 0,3X = 1y,X(+3) + y(-1) = 0,1,Choose the lowest set of integers that satisfies the equation,(C2H3O2)3,If there is only one atom the “1” is not shown,Next,Example #4-Names to Formulas,lithium phosphate,Li,PO4,2. Determi
31、ne number of ions,1. Write symbols of elements,Final Formula,(Li )x(PO4-3)y= 0,1X = 3y,X(+1) + y(-3) = 0,3,+1,Choose the lowest set of integers that satisfies the equation,(PO4)1,If there is only one atom the “1” is not shown,If there is no Roman Numeral, you need to know the fixed oxidation number
32、of the positive ion.,If there is no Roman Numeral, you need to know the fixed oxidation number of the positive ion.,Next,Practice Problems,By now you should have an idea of what is expected when naming covalent binary compounds using prefixes.In order to master this naming system you need to practic
33、e until you feel proficient in naming compounds using prefixes.,Practice Problem #1,Fe(NO3)3,Choose the correct name for the compound,1. Iron trinitrate,2. iron(I) nitrate,3. iron(III) nitrite,4. iron(III) nitrate,5. none of the above,No, you have the wrong oxidation number,No, you need to review po
34、lyatomic ions,Very good, click arrow to continue,No, there is a correct answer,No, you do not use prefixes,next problem,Polyatomic Ions,Periodic Chart,Practice Problem #2,sodium chlorite,Choose the correct formula for the compound,1. NaCl,2. NaClO,3. NaClO2,4. Na(ClO)2,5. none of the above,No, you n
35、eed to review prefixes,Very good, click arrow to continue,No, you have several errors,No, there is a correct answer,No, you need to review prefixes,next problem,Prefixes,Periodic Chart,POLYATOMIC IONS,Ions with -1 charge perbromate BrO4-1 bromate BrO3-1 bromite BrO2-1 hypobromite BrO-1 perchlorate C
36、lO4-1 chlorate ClO3-1 chlorite ClO2-1 hypochlorite ClO-1 periodate IO4-1 iodate IO3-1 iodite IO2-1 hypoiodite IO-1,nitrate NO3-1 nitrite NO2-1 hydroxide OH-1 cyanide CN-1 thiocyanate SCN-1 acetate C2H3O2-1 Permanganate MnO4-1 bicarbonate HCO3-1Ions with a -2 Charge carbonate CO3-2 phthalate C8H4O4-2
37、 sulfate SO4-2,sulfite SO3-2 chromate CrO4-2 dichromate Cr2O7-2 oxalate C2O4-2 peroxide O2-2Ions with a -3 Charge phosphate PO4-3 phosphite PO3-3 arsenate AsO4-3Ions with +1 charge ammonium ion NH4+1,return,N,Oxidation Numbers (most common),La,Hf,Ta,Re,Os,Ce,Ba,Tl,Pb,Bi,Po,At,Rn,Ir,Pt,Au,Hg,Y,Zr,Nb,
38、Mo,Tc,Ru,Rb,Sr,In,Sn,Sb,Te,I,Xe,Rh,Pd,Ag,Cd,Sc,Ti,V,Cr,Mn,Fe,K,Ca,Ga,Ge,As,Se,Br,Kr,Co,Ni,Cu,Zn,Al,Si,P,S,Cl,Ar,Na,Mg,B,C,O,F,Ne,Li,Be,H,H,He,Ac,Rf,Db,Sg,Rh,Hs,Fr,Ra,Mt,+1,+2,+3,1A,2A,8A,0,-4,-3,-2,-1,7A,6A,5A,4A,3A,W,Nd,Pm,Sm,Eu,Gd,Tb,Ce,Pr,Yb,Lu,Dy,Ho,Er,Tm,Np,Am,Cm,Bk,Th,Pa,No,Lr,Cf,Es,Fm,Md,U,Pu,Click on element to see its oxidation number(s),return,
